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First law of thermodynamics states that $$\tag{1} dU=\delta Q + \delta W$$

whereas second law of thermodynamics states that, for a reversible process, $$\tag{2} dS= \frac{\delta Q}{T} $$

I have also seen $(1)$ and $(2)$ expressed in terms of variations, as follows:

$$\tag{3} \Delta U=\Delta Q + \Delta W$$

$$\tag{4} \Delta S= \frac{\Delta Q}{T} $$

In bothy equations $(1)$ and $2$ appears the inexact differential symbol, $\delta$, so I assume that those variables labelled with the $\delta$ need an integrating factor to be solved. However, it seems that the new equations have been achieved simply by performing an integral.

Then,

  1. How are these equations transformed from their differential forms to their integral ones?

  2. Are $(3)$ and $(4)$ as general $(1)$ and $(2)$, or they can be used only under certain conditions?

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    $\begingroup$ What do you mean by them needing an "integrating factor to be solved"? You can integrate inexact differentials also paths without any problems, and in fact that they are integratable along path may be seen as their defining characteristic, see physics.stackexchange.com/a/96095/50583 $\endgroup$
    – ACuriousMind
    Jan 12, 2020 at 19:52
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    $\begingroup$ While eq. (1) and (2) are sophisticated expressions eq. (3) and (4) are often used in high school or in the first year during university. I take them as "quantitative expressions" (except for special cases) and use them to get covey a "first idea" of what is going on. $\endgroup$
    – Semoi
    Jan 12, 2020 at 20:30
  • $\begingroup$ @ACuriousMind♦ ok thanks, I misunderstood the concept $\endgroup$
    – Quaerendo
    Jan 13, 2020 at 11:48

1 Answer 1

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First law of thermodynamics states that 𝑑𝑈=𝛿𝑄+𝛿𝑊

The symbol 𝛿 is used instead of $d$ to represent inexact differentials because heat $Q$ and work $W$ are path dependent, whereas $d$ is the exact differential used for $U$ (internal energy) is not path dependent, i.e., it is a system property. According to Wikipedia the convention to use 𝛿 originated in the 19th century work of German mathematician Carl Gottried.

Although work and heat are path dependent, the combination of the two is not as they determine the change in internal energy, which is path independent. This is the reason the following form can be used.

$$\Delta U=Q+W$$

The more precise definition of entropy is

$$dS=\frac{𝛿Q_{rev}}{T}$$

Where the suffix $rev$ means heat transfer for a reversible path.

The form

$$\Delta S=\frac{Q}{T_{reservoir}}$$

Can be used when the heat transfer occurs at constant temperature, such as transfer with a heat reservoir, so that temperature can come out of the integral when integrating the differential form.

Hope this helps.

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